H2PO4 (-)
Dihydrogen Phosphate
C2H3O2 (-)
Acetate
HSO3 (-)
Hydrogen Sulfite
HSO4 (-)
Hydrogen Sulfate
HCO3 (-)
Hydrogen Carbonate
NO2 (-)
Nitrite
NO3 (-)
Nitrate
CN (-)
Cyanide
OH (-)
Hydroxide
MnO4 (-)
Permanganate
ClO (-)
Hypochlorite
ClO2 (-)
Chlorite
ClO3 (-)
Chlorate
ClO4 (-)
Perchlorate
HPO4 (2-)
Hydrogen Phosophate
SO3 (2-)
Sulfite
SO4 (2-)
Sulfate
CO3 (2-)
Carbonate
CrO4 (2-)
Chromate
Cr2O7 (2-)
Dichromate
SeO4 (2-)
Selenate
SiO3 (2-)
Silicate
C4H4O6 (2-)
Tartrate
AsO4 (3-)
Arsenate
S2O3 ()2-
Thiosulfate
BO3 (3-)
Borate
B4O7 (2-)
Tetraborate
SiF6 (2-)
Hexaflorosilicate
SCN (-)
Thiocynate
IO4 (-)
Periodate
IO3 (-)
Iodate
IO (-)
Hypoidate
NH2 (-)
Amide
C2O4 (2-)
Oxalate
HC2O4 (-)
Hydrogen Oxalate
NH3
Ammonia
NH4 (+)
Ammonium
O2 (2-)
Peroxide
PO4 (3-)
Phosphate
PO3 (3-)
Phosphite
BrO3 (-)
Bromate
BrO (-)
Hypobromite
Li (+)
Lithium Ion
Na (+)
Sodium Ion
K (+)
Potassium Ion
Rb (+)
Rubidium Ion
Cs (+)
Cesium Ion
Fr (+)
Francium Ion
Be (2+)
Beryllium Ion
Mg (2+)
Magnesium Ion
Ca (2+)
Calcium Ion
Sr (2+)
Strontium Ion
Ba (2+)
Barium Ion
Ra (2+)
Radium Ion
N (3-)
Nitrogen Ion
P (3-)
Phosphorus Ion
As (3-)
Arsenic Ion
Sb (3-)
Antimony Ion
Bi (3-)
Bismuth Ion
O (2-)
Oxygen Ion
S (2-)
Sulfur Ion
Se (2-)
Selenium Ion
Te (2-)
Tellurium Ion
Po (2-)
Polonium Ion
F (-)
Fluorine Ion
Cl (-)
Chlorine Ion
Br (-)
Bromine Ion
I (-)
Iodine Ion
At (-)
Astatine Ion
An alternative term that can be used when referring to the charge of an atom, but not a polyatomic ion. (There is a technical difference)
Definition: Oxidation State
An element which has the capacity to act as either a metal or nonmetal, depending on the chemical circumstances
Definition: Metalloid
An elements that gains electrons, becoming negatively charged, see anion.
Definition: Nonmetal
An element that tens to lose electrons, becoming positively charged, see cation
Definition: Metal
An atom of group of atoms either positively or negatively charged
Definition: Ion
Positively charged ion.
Definition: Cation
Negatively charged ion
Definition: Anion
A single atom ion (ex. Na+ and Cl-)
Definition: Monatomic Ion
An ion made up of many atoms (Poly means many) which acts chemically as one unit.
Definition: Polyatomic Ion
A compound containing at east one ionic bond (a metal and a nonmetal bond)
Definition: Ionic Compound
A compound containing only covalent bonds. Known as “real” molecules. They contain only nonmetal atoms.
Definition: Covalent Compound
An ionic compound with only 2 kinds of atoms
Definition: Binary Ionic Compound
A covalent compound with only 2 kinds of atoms
Definition: Binary Molecular Compound
Metal
Cations have the same name as the ____
Roman Numerals
Metals that can form cations of different charges are followed by _____
-ium
Cations formed from nonmetal atoms end in
H3O (+)
Hydronium Ion
-ide
Monatomic anions end in
-ate (most common oxyanion) & -ite (one less O atom that the most common oxyanion)
Polyatomic anions containing oxygen end in
(two endings*)
(two endings*)
one more O atom than the anion ending in -ate
The prefix per- indicates
one less O atom than the anion ending in -ite
The prefix hypo- indicates
hydrogen or dihydrogen
Anions derived by adding H+ to an oxyanion use ____ or ____ as a prefix
-ide (examples Cyanide, Hydroxide, Peroxide)
Exception to the rule: a few simple polyatomic anions end in
the anion name
Binary Ionic Compounds consist of the cation name followed by…
-ous for the lower charge
-ic for the higher charge
-ic for the higher charge
Alternatively the common name may be used if a metal has more than one possible ion. Here, use the Latin root and add _____ for the lower charge and ____ for the higher charge
-ic
Acids: anions that end in -ide are changed to end with
-ite and -ous
Acids: anions that end in -ate or -ite are changed to end with
HCl
Hydrochloric Acid
HF
Hydrofluoric Acid
H2S
Hydrosulfuric Acid
HNO3
Nitric Acid
HNO2
Nitrous Acid
HClO4 (-)
Perchloric Acid
HClO3 (-)
Chloric Acid
HClO2 (-)
Chlorous Acid
HClO (-)
Hypochlorous Acid
H2SO4
Sulfuric Acid
Hydro-
Acids: add ____ as a prefix when the acid does not have oxygen
mono-
Covalent prefix for 1 atom
di-
Covalent prefix for 2 atoms
tri-
Covalent prefix for 3 atoms
tetra-
Covalent prefix for 4 atoms
penta-
Covalent prefix for 5 atoms
hexa-
Covalent prefix for 6 atoms
hepta-
Covalent prefix for 7 atoms
octa-
Covalent prefix for 8 atoms
nona-
Covalent prefix for 9 atoms
deca-
Covalent prefix for 10 atoms
NO
Nitrogen monoxide
N2O
Dinitrogen monoxide
NO2
Nitrogen dioxide
N2O5
Dinitrogen pentoxide
Cl2O
Dichlorine monozide
NF3
Nitrgen Triflouorine
CO
Carbon monoxide
CO2
Carbon Dioxide
Do not add mono at the beginning of a covalent molecule if the compound’s first atom is only 1.
Covalent compound rule:
Copper (I)
Cu (+)
Copper (II)
Cu (2+)
Iron (II)
Fe (2+)
Iron (III)
Fe (3+)
Tin (II)
Sn (2+)
Tin (IV)
Sn (4+)
Nickel (II)
Ni (2+)
Nickel (IV)
Ni (4+)
Chromium (II)
Cr (2+)
Chromium (III)
Cr (3+)
Manganese (II)
Mn (2+)
Manganese (III)
Mn (3+)
Mercury (I)
Hg2 (2+)
Mercury (II)
Hg (2+)
Lead (II)
Pb (2+)
Lead (IV)
Pb (4+)
Cobalt (II)
Co (2+)
Cobalt (III)
Co (3+)
Gold (I)
Au (+)
Gold (III)
Au (3+)
CF6
Carbon Tetrafluorine
P2O5
Diphosphorus pentoxide
PF3
Phosphorus trifluoride
N2O4
Dinitrogen tetroxide
SO2
Sulfur Dioxide
SO3
Sulfur Trioxide
SF6
sulfur hexafluoride
CCl4
carbon tetrachloride
NI3
nitrogen triiodide
PCl3
Phosphorus trichloride
PBr3
Phosphorus tribromide
NCl3
Nitrogen trichloride
Br2O
dibromide oxide
I2O
diiodide oxide
dot
In a hydrate, water and the compound is separated by a
covalent compounds
hydrates use the same prefixes as
copper(II) sulfate pentahydrate.
CuSO4•5H2O
Na2CO3•10H2O
sodium carbonate decahydrate
MgSO4•7H2O
magnesium sulfate heptahydrate
CdSO4•8H2O
cadmium sulfate octahydrate
LiClO4•3H2O
lithium perchlorate trihydrate
